Molarity equations

Mass (g)

Amount (mol) × Molar Mass (g/mol)\

Amount (mol)

Mass (g) ÷ Molar Mass (g/mol)

Molar Mass (g/mol)

Mass (g) ÷ Amount (mol)

Number of Particles

Amount (mol) × 6.022 × 10^23\

Amount (mol) from Particles

Number of Particles ÷ (6.022 × 10^23)\

Number of Atoms

Amount (mol of atoms) × 6.022 × 10^23)

Number of Molecules

Amount (mol of molecules) × 6.022 × 10^23\

Number of Formula Units

Amount (mol of ionic compound) × 6.022 × 10^23\

Number of Molecules

[Mass (g) ÷ Molar Mass (g/mol)] × (6.022 × 10^23)

Mass (g) from Number of Particles

[Number of Particles ÷ (6.022 × 10^23)] × Molar Mass (g/mol)\

Moles of Element Atoms

Moles of Compound × Number of That Element's Atoms per Formula Unit\

Moles of Compound from Moles of Element Atoms

Moles of Element Atoms ÷ Number of That Element's Atoms per Formula Unit\

Number of Element Atoms from Moles of Compound

Moles of Compound × Atoms of Element per Formula Unit × 6.022 × 10^23\

Moles of Element Atoms from Mass of Compound

[Mass of Compound (g) ÷ Molar Mass of Compound (g/mol)] × Atoms of Element per Formula Unit\

Mass of Element (g)

Moles of Element Atoms × Atomic Molar Mass (g/mol)\

Mass of Element in Compound (g)

[Mass of Compound (g) ÷ Molar Mass of Compound (g/mol)] × Atoms of Element per Formula Unit × Atomic Molar Mass (g/mol)

Percent Composition of Element

(Mass of Element in 1 mol of Compound ÷ Molar Mass of Compound) × 100%\

Mass of Element (g) from Percent Composition

Mass of Compound (g) × (Percent Composition ÷ 100)

Moles of Each Element for Empirical Formula

Mass of Each Element (g) ÷ Atomic Molar Mass (g/mol)

Empirical Formula

Moles of Each Element ÷ Smallest Number of Moles Among the Element